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Why does the element with lowest atomic number have the greatest atomic radii in each period?
Across the period, the total number of shells remain the same. But, atomic number, i.e., no. of protons and electrons goes on increasing. Protons (positively charged) present in the nucleus exert a nuclear charge towards the electrons (negatively charged) present around the nucleus, and pull the shells toward the nucleus. Hence, when no. of protons increases, nuclear charge also increases and hence it pulls the shells with greater force, and shells get closer to the nucleus. Hence, across the period, atomic size, or the radii go on decreasing.
Does atomic radius have a bigger atomic number as you go to the right of the periodic table?
Yes. Generally atomic radii turn to decrease as you move across the periodic table from left to right. this is because the nuclear charge increases as you move right across the period but the electron screening remains the same. consequently, the protons in the nucleus has a greater pull on the electrons.
How do you account for the general trend in atomic radius across a row of elements?
The general trend in atomic radius across a row of elements decreases from left to right due to increasing effective nuclear charge, which attracts the electrons closer to the nucleus. As you move across a period, the number of protons in the nucleus increases, resulting in a stronger pull on the electrons and a decrease in atomic radius. Additionally, the shielding effect of inner electrons remains relatively constant, further contributing to the trend.
What happens to the atomic radius as you go across a period?
It decreases as you move from left to right because there is an increase in positive charge in the nucleus as you go from left-to-right. Each time you go over an element it has one more electron and proton added to the principal energy level, so the nucleus pull increases and it holds the valence electron in tighter.
What happen to the atomic as you from the bottom to the top of the periodic table?
As you move from the bottom to the top of the periodic table, the atomic size decreases. This is because the number of protons in the nucleus increases, leading to a stronger pull on the electrons. Electrons are added to the same energy level while moving up the table, resulting in a smaller atomic radius.
Which has more potential energy an electron close to an atomic nucleus or one far from an atomic nucleus?
An electron far from an atomic nucleus has more potential energy compared to one close to the nucleus. This is because the farther the electron is from the nucleus, the higher its potential energy due to the increased distance from the attraction of the positively charged nucleus.
Why does the atomic radius decrease with an increase in atomic numbers within a period?
As the atomic number increases, the number of protons in the nucleus increases or the effective nuclear charge of the nucleus increases. As a result the force exerted by the nucleus on the valence electrons is more or the size of the atom is small.
When moving left to right across the periodic table the atomic number increases and the atomic radius?
The atomic radius decreases from left to right and increases from top to bottom
Why does the element with lowest atomic number have the greatest atomic radii in each period?
Across the period, the total number of shells remain the same. But, atomic number, i.e., no. of protons and electrons goes on increasing. Protons (positively charged) present in the nucleus exert a nuclear charge towards the electrons (negatively charged) present around the nucleus, and pull the shells toward the nucleus. Hence, when no. of protons increases, nuclear charge also increases and hence it pulls the shells with greater force, and shells get closer to the nucleus. Hence, across the period, atomic size, or the radii go on decreasing.
What has greater pull by nucleus electron in outer shell of neon or sodium?
The nucleus of sodium has a greater pull on the electron in the outer shell compared to the nucleus of neon. This is because sodium has one less electron in its outer shell than neon, resulting in a stronger attraction between the nucleus and the remaining electron in sodium.
Why does atomic radii decrease moving left to right across a period?
Atomic radii decrease moving left to right across a period because as you move from left to right, the number of protons in the nucleus increases, leading to a greater nuclear pull on the electrons. This increased nuclear attraction pulls the electrons closer to the nucleus, resulting in a smaller atomic radius.
Why does the electronegativity increase as the atomic number increases?
The number of electrons increases with the atomic number. So the electronegativity increases with the atomic number. Not quite. Electronegativity doesn't consistently increase with atomic number. For example, F is more electronegative than Na, even though Na has a higher atomic number.
Why fluorine has smaller atomic radius than both oxygen and chlorine?
Fluorine has more electronegativity, meaning it is more "desperate" to obtain electrons. Its nucleus is the most attractive of all elements.
Why does potassium have a larger atomic radius than bromine?
When looking at potassium and bromine, it would seem that with more electrons occupying more orbitals, bromine would be larger. However, in addition to those additional electrons, bromine also has additional protons. These protons in the nucleus pull on all of bromine's electrons with more strength than the nucleus of potassium, and the stronger pull offsets any size gained by adding electrons. In short, bromine's nucleus pulls harder.
Does atomic radius have a bigger atomic number as you go to the right of the periodic table?
Yes. Generally atomic radii turn to decrease as you move across the periodic table from left to right. this is because the nuclear charge increases as you move right across the period but the electron screening remains the same. consequently, the protons in the nucleus has a greater pull on the electrons.
How do you account for the general trend in atomic radius across a row of elements?
The general trend in atomic radius across a row of elements decreases from left to right due to increasing effective nuclear charge, which attracts the electrons closer to the nucleus. As you move across a period, the number of protons in the nucleus increases, resulting in a stronger pull on the electrons and a decrease in atomic radius. Additionally, the shielding effect of inner electrons remains relatively constant, further contributing to the trend.
What happens to the atomic radius as you go across a period?
It decreases as you move from left to right because there is an increase in positive charge in the nucleus as you go from left-to-right. Each time you go over an element it has one more electron and proton added to the principal energy level, so the nucleus pull increases and it holds the valence electron in tighter.
